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Journal of Alloys and Compounds 338 (2002) 87–92 L www.elsevier.com / locate / jallcom Synthesis, characterization and bonding of Ba 3 Li 4 Sn 8 Svilen Bobev, Slavi C. Sevov* Department of Chemistry and Biochemistry, University of Notre Dame, Notre Dame, IN 46556, USA Received 18 October 2001; accepted 26 November 2001 Abstract The ternary compound Ba 3 Li 4 Sn 8 was obtained by slow cooling of a stoichiometric mixture of the elements that was heated at 800 8C ˚ V5833.2(2) A ˚ 3 , R 1 /wR 2 5 4.03 / 11.33%) for 2 days. Its structure (monoclinic, C2 /m, Z52, a518.549(1), b56.685(1), c56.792(1) A, 1 102 contains one-dimensional chains of ` [Sn 8 ] made of edge-sharing cyclodecane-like units in their ‘all-chair’ conformations. The cations screen the chains from each other and provide the extra electrons needed for bonding in the chains. The structure and the electron count can be rationalized in terms of the Zintl concept as (Ba 21 ) 3 (Li 1 ) 4 [(2b-Sn 22) 2 (3b-Sn 12) 6 ], i.e. the compound is an electronically balanced, Zintl phase. Nevertheless, Ba 3 Li 4 Sn 8 exhibits temperature-independent paramagnetism that is, most likely, of van Vleck type as a result of the very small band gap of about 0.3 eV. 2002 Elsevier Science B.V. All rights reserved. Keywords: Intermetallic; Zintl phases; X-ray diffraction; Electronic band structure 1. Introduction The discovery of Tt 42 in neat solids (Tt5Tetrel, 9 ] ] element of group 14) stimulated the search for Zintl phases with other isolated clusters, either new or similar to those known as crystallized from solutions [1–6]. Our thorough and systematic studies of the binary A–Tt systems (A5 alkali metal) extended into the pseudo-binary systems with mixed alkali metals, especially combinations of very different sizes, and provided the first arachno-clusters of group 14, Sn 62 in A 4 Li 2 Sn 8 for A5K or Rb [7]. Similar8 ly, germanium forms novel giant clusters, truncated tetrahedra of Ge 122 12 , when combined with a mixture of Li and Rb in RbLi 7 Ge 8 [8]. It is important to emphasize that both novel species form only in Li-containing, mixed alkalimetal phases, and not in simple binaries. Besides the role of the sizes of the cations these phases are apparently stabilized also by the better covalency of lithium which caps the open faces of these clusters and stabilizes them as closo-species, Li 2 Sn 42 and Li 4 Ge 82 8 12 [7,8]. Also, mixed alkali metals provide compounds with isolated clusters of 42 lead, Pb 42 of different shapes [9]. 4 -tetrahedra and Pb 9 Following the studies of the pseudo-binary systems with mixed alkali metals we have taken one step further in complexity and have studied the systems alkali-metal (A)– alkaline-earth metal (AE)–tetrel (Tt). Found in these systems were truncated tetrahedra of Sn 122 in 12 [AE]Na 10 Sn 12 for AE5Ca or Sr [10], and similar to the 82 lithium-stabilized closo-Li 4 Ge 12 , they are stabilized by 82 sodium as closo-Na 4 Sn 12 clusters. Using Ba instead of Ca or Sr led to the formation of the largest naked cluster of a main-group element, Sn 442 in Ba 16 Na 204 Sn 310 [11]. This 56 cluster is made of four fused pentagonal dodecahedra of tin that are stuffed with four barium cations. Here we report the synthesis and structural characterization of another compound with mixed alkali and alkaline-earth cations, Ba 3 Li 4 Sn 8 . It exhibits one-dimensional chains of 1 102 that are made of edge-sharing cyclodecane-like ` [Sn 8 ] units in their ‘all-chair’ conformation, unprecedented structural motifs in the chemistry of the heavier carbon homologues. 2. Experimental section 2.1. Synthesis *Corresponding author. Tel.: 11-219-631-5891; fax: 11-219-6316652. E-mail address: [email protected] (S.C. Sevov). All manipulations were performed in an Ar-filled glove box. The surfaces of Li (rod, Aldrich, 99.9%, sealed under 0925-8388 / 02 / $ – see front matter 2002 Elsevier Science B.V. All rights reserved. PII: S0925-8388( 02 )00219-0 88 S. Bobev, S.C. Sevov / Journal of Alloys and Compounds 338 (2002) 87 – 92 Ar) and Ba (rod, Alfa, 99.2%, sealed under Ar) were cleaned off with a scalpel immediately before use, while Sn (rod, Alfa, 99.999%) was used as received. All reactions were carried out in sealed niobium tubes, which were in turn jacketed and sealed under vacuum in silica ampoules. More details on the techniques and the procedures are described elsewhere [12]. Initially, Ba 3 Li 4 Sn 8 was synthesized as the major product of a reaction designed to produce BaLi 10 Sn 12 , the barium–lithium analog of [AE]Na 10 Sn 12 (AE5Ca, Sr) [10]. The reaction was carried out at 800 8C (m.p. of Ba is 725 8C; no phase diagram for Ba–Sn; the highest m.p. in Li–Sn is 780 8C) for 48 h and cooled down to room temperature with a rate of 5 8C / h. Other products from that reaction, as identified by powder X-ray diffraction (EnrafNonius Guinier camera with a vacuum chamber and Cu Ka radiation), were traces of BaSn 3 and LiSn as well as some unreacted Sn metal. After the stoichiometry of the compound was obtained from the structure determination, stoichiometric mixtures were treated at the same temperature regimes. A least-squares refinement of the measured 2u values of the X-ray powder diffraction pattern of the compound relative to those of the internal standard (silicon) verified the lattice constants. 2.2. Structure determination Numerous crystals of Ba 3 Li 4 Sn 8 were selected in the glove box and were sealed in 0.2 mm thin-walled glass capillaries. They were checked for singularity on an EnrafNonius CAD4 single-crystal diffractometer (graphite˚ One of monochromated Mo Ka radiation, l 50.71073 A). these crystals (irregular, 0.1630.1430.08 mm) was chosen and a unique quadrant of X-ray diffraction data was collected at room temperature with v –2u scans and up to 2u of 608. All 2013 reflections were corrected for absorption with the aid of the average of c-scans of four reflections at different u angles (R int 50.051; T min /T max 5 0.154 / 0.316). The observed extinction conditions and the intensity statistics suggested the centrosymmetric space group C2 /m. Consequently, the structure was successfully solved and refined with the aid of the SHELXTL-V5.1 software package [13] in that space group. The direct methods provided three peaks with distances to each other appropriate for tin atoms, and two peaks with distances to the other three that were appropriate for barium atoms, and they were all so assigned. The following least-squares cycles and a difference Fourier synthesis revealed two peaks at special positions and with relatively low heights. These were assigned as lithiums, and the subsequent anisotropic refinement of all atoms converged at R 1 5 4.17%; wR 2 5 11.43% for 1309 independent reflections and 43 parameters. Further details on the data collection and refinement parameters are summarized in Table 1, while positional and equivalent isotropic displacement Table 1 Selected data collection and refinement parameters for Ba 3 Li 4 Sn 8 Chemical formula Formula weight Space group, Z ˚ Unit cell parameters (A) Ba 3 Li 4 Sn 8 1389.30 C2 /m (No. 12), 2 a518.549(1) b56.685(1) c56.792(1) b 598.34(1)8 ˚3 V 5 833.2(2) A Mo Ka, 0.71073 608 186.84 5.538 1309 / 0 / 43 R 1 5 4.03%, wR 2 5 11.33% R 1 5 4.17%, wR 2 5 11.43% ˚ Radiation, l (A) 2u limit m (cm 21 ) rcalcd (g / cm 3 ) Data / restraints / parameters R indices (I . 2sI )a R indices (all data) a R 1 5 ouuFo u 2 uFc uu / ouFo u; wR 2 5 [o[w(F o2 2 F c2 )2 ] / o[w(F o2 )2 ]] 1 / 2 . w 5 1 / [s 2 F o2 1 (0.0673P)2 1 29.333P], P 5 (F o2 1 2F c2 ) / 3. parameters and important distances are listed in Tables 2 and 3, respectively. 2.3. Magnetic measurements The magnetizations of different samples of Ba 3 Li 4 Sn 8 were measured on a Quantum Design MPMS SQUID magnetometer at a field of 30 kG over the temperature range 10–280 K. Measurements at lower temperatures (down to 4 K) and lower magnetic fields of 50, 100 and 300 G were carried out as well. The samples were contained in special holders designed for air-sensitive compounds [12]. The raw data were corrected for the holder contribution and for ion-core diamagnetism. The corrected magnetic susceptibility is positive and temperature independent, and varies between 4.17310 24 and 4.98310 24 emu / mol (average of two measurements on two different samples). No superconductivity was observed at the low temperatures and magnetic fields. 2.4. Band calculations ¨ Extended Huckel band calculations were carried out within the tight binding approximation with only the tin atoms included (Hii and z1 for Sn 5s: 216.16 eV and 2.12, for Sn 5p: 28.32 eV and 1.82) [14]. The density of states Table 2 Atomic coordinates and equivalent isotropic displacement parameters ˚ 2 ) for Ba 3 Li 4 Sn 8 (A Atom Site x y z Ueq Sn1 Sn2 Sn3 Ba1 Ba2 Li1 Li2 4i 4i 8j 2a 4i 4h 4i 0.12920(4) 0.48483(4) 0.85055(3) 0 0.32245(4) 0 0.209(1) 0 0 0.73248(8) 0 0 0.787(4) 0 0.4541(1) 0.2020(1) 0.19789(8) 0 0.6913(1) 1/2 0.130(4) 0.0142(2) 0.0145(2) 0.0141(2) 0.0135(2) 0.0153(2) 0.029(5) 0.022(4) S. Bobev, S.C. Sevov / Journal of Alloys and Compounds 338 (2002) 87 – 92 89 Table 3 ˚ and angles (8) in Ba 3 Li 4 Sn 8 Important bond distances (A) Sn1– 23 23 23 Sn2– 23 23 23 Sn3– Sn3–Sn1–Sn3 Sn2–Sn2–Sn3 Sn3–Sn2–Sn3 Sn3 Li1 Li2 Ba1 Ba2 Ba2 Sn2 Sn3 Li1 Ba1 Ba2 Sn1 Sn2 Sn3 Li1 Li2 Li2 Ba1 Ba2 Ba2 Ba2 2.9440(9) 2.84(1) 2.82(2) 3.6211(9) 3.6342(6) 3.711(1) 2.880(2) 2.9325(8) 2.77(2) 3.6393(6) 3.543(1) 2.9440(9) 2.9325(8) 3.108(1) 3.221(3) 2.94(2) 3.03(2) 3.7107(6) 3.7422(9) 3.7977(9) 3.8421(8) 74.81(3) 105.90(4) 64.00(3) Li1– 23 23 23 23 Li2– Ba1– Ba2– 23 23 23 23 43 23 43 23 23 23 23 23 Sn2–Sn3–Sn1 Sn2–Sn3–Sn3 Sn1–Sn3–Sn3 Sn1 Sn2 Sn3 Li1 Ba1 Sn1 Sn3 Sn3 Ba2 Sn1 Sn2 Sn3 Li1 Sn1 Sn1 Sn2 Sn3 Sn3 Sn3 Li2 2.84(1) 2.77(2) 3.221(3) 2.85(6) 3.68(1) 2.82(2) 2.94(2) 3.03(2) 3.630(9) 3.6211(9) 3.6393(6) 3.7107(6) 3.68(1) 3.6342(6) 3.711(1) 3.543(1) 3.7422(9) 3.7977(9) 3.8421(8) 3.630(9) 107.75(3) 58.00(1) 127.40(2) and the crystal orbital overlap populations were calculated on the basis of 240 k-points over the irreducible wedge of the Brillouin zone. 3. Results and discussion Fig. 1. General view of the C-centered monoclinic structure of Ba 3 Li 4 Sn 8 viewed: (a) along the b axis, and (b) along the c axis. The large and small isolated spheres are Ba and Li atoms, respectively. The unit cell is outlined. 3.1. Structure description The structure of Ba 3 Li 4 Sn 8 consists of isolated chains of tin that run along the b axis of the monoclinic cell (Fig. 1). The repeating monomeric unit of the chains is cyclodecane in its ‘all-chair’ conformation (Fig. 2). Each monomer shares two directly opposite edges with its two neighbors in the chain. Interestingly, there is another compound in the ternary (AE)–Li–Tt system with almost the same composition, Ca 31x Li 42x Si 8 [15], and its structure, although different from Ba 3 Li 4 Sn 8 , contains also chains of the tetrel. The difference is that the chains of silicon are made of interconnected xylene-like rings rather than fused cyclodecanes. The cyclodecanes in Ba 3 Li 4 Sn 8 are made of three unique tin sites (Fig. 2), two of which, Sn2 and Sn3, are three-bonded, while the third, Sn1, is two-bonded. The Sn–Sn distances within the cyclodecane monomer are ˚ (Table 3). They are quite similar, 2.880(2)–2.9440(9) A typical for single, localized Sn–Sn bonds such as those found in Sn 42 tetrahedra and 1` [Sn] 22 zigzag chains [16]. 4 The edges that are shared with neighboring cyclodecanes are Sn2–Sn2 pairs. This brings the Sn3 atoms (the atoms next to the shared edges) of different cyclodecanes in ˚ Thus, a triangle of one relatively close proximity, 3.108 A. Sn2 and two Sn3 atoms is formed when the Sn3–Sn3 Fig. 2. An ORTEP drawing (80% probability thermal ellipsoids) of a three-monomer section of the 1` [Sn 8 ] 102 chain. The monomer is with the shape of a cyclodecane in its ‘all-chair’ conformation (outlined). Each cyclodecane shares two opposite edges with two neighbors. 90 S. Bobev, S.C. Sevov / Journal of Alloys and Compounds 338 (2002) 87 – 92 ˚ is considered. This distance is contact of 3.108(1) A somewhat longer but compares well with the distances in ˚ [16], in BaSn 3 with metallic b-Sn, 3.016 and 3.175 A ˚ [17], and in isolated triangular Sn 322 units, 3.058 A 122 Ca 31 Sn 20 with Sn 62 dimers and Sn linear pentamers, 2 5 ˚ [18], and should be considered in the 3.063–3.158 A bonding picture. Longer distances in lithium-containing compounds have been discussed extensively elsewhere ˚ relative [19]. The elongation, usually in the order of 0.15 A to Sn–Sn single-bond distance, is explained by the strong cation field effects and strong polarizing power of lithium [19]. The angles at the tin atoms deviate substantially from the ideal tetrahedral angle and are in a very wide range, all the way from 58.00(1) to 107.75(3)8. As might be expected, the sharpest angles are within the isosceles triangle of two Sn3 and one Sn2 atoms, 58.00(1) and 64.00(3)8. These are followed by the angle at the twobonded Sn1, 74.81(3)8, for which a relatively small angle is normal due to the two lone pairs of electrons associated with it. The remaining angles are closer to tetrahedral. It should be pointed out that isolated triangular units of Sn 22 3 with two delocalized p electrons that are isoelectronic with the aromatic cyclopropenium cation C 3 H 31 exist in BaSn 3 [18]. 3.2. Electronic structure The electron needs for bonding in the chains can be discerned based on the octet rule. Thus, a three-bonded pyramidal atom such as Sn2 and Sn3 carries a lone pair of electrons and must provide an electron for each bond, or a total of five electrons per atom. A two-bonded atom such as Sn1 carries two lone pairs of electrons in addition to the two electrons of the two bonds, or a total of six electrons. This means that the formal oxidation state for Sn2 and Sn3 is 12 while for Sn1 it is 22. Thus, the need of additional electrons for the bonding of the repeating unit of two Sn1, two Sn2, and four Sn3 atoms becomes 23(22)123(12) 143(12)5102. Exactly that many electrons are available from the three Ba and four Li atoms in the formula of the compound, Ba 3 Li 4 Sn 8 , and therefore the compound should be electronically-balanced, or a Zintl phase. This simple counting scheme assumes, of course, complete electron transfer from the alkali and alkaline-earth metals to the post-transition element. However, it does not provide insight into the electron distribution among the different Sn–Sn bonds or the strength of the different interactions. Furthermore, actual negative charges rarely correspond to the assigned formal oxidation states. In order to study the bonding of Ba 3 Li 4 Sn 8 in more detail and to eventually relate its structure to the observed temperature¨ independent paramagnetism, extended Huckel band calculations were carried out for the Sn sublattice. The total density of states (DOS) is shown in Fig. 3 together with Fig. 3. Shown are the total DOS (black line), the projected partial DOS of Sn3 (gray line), and the Fermi level (broken line) for Ba 3 Li 4 Sn 8 . A very small band gap of less than 0.3 eV separates the valence and conduction bands. the projected partial DOS of Sn3. The total of 42 electrons for the repeating unit Sn 102 fill the bands below the Fermi 8 level at 25.12 eV. Thus, the valence band is completely filled and is separated by a very narrow gap of less than 0.3 eV from the conduction band. This suggests that the observed temperature-independent paramagnetism of Ba 3 Li 4 Sn 8 is either of van Vleck type, i.e. paramagnetism due to mixing of the ground state (filled valence band) with thermally-empty, yet low-lying, excited paramagnetic states (conduction band), or that simply the conduction and valence bands overlap. The latter is quite possible because, ¨ as it is well known, extended-Huckel calculations are only an approximation and often overestimate the band gaps. Furthermore, we should keep in mind that the calculations did not include the cation–anion interactions, which will further perturb the overall widths and positions of the valence and conduction bands, and may very well cause overlap between them. These interactions, especially with lithium may have significant covalent character as already pointed out. S. Bobev, S.C. Sevov / Journal of Alloys and Compounds 338 (2002) 87 – 92 Closer look at the DOS (Fig. 3) indicates that, as expected, the bands below 212.8 eV are the tin s states while the valence band, between 25.12 and 211.2 eV, is predominantly tin p states. In order to evaluate further the bonding in this compound, we calculated crystal orbital overlap population (COOP) curves for the different Sn–Sn interactions (Fig. 4). They showed that the main bonding states occur within the largest peak of the valence band in the DOS, between 211 and 28 eV, while the states of the same band above 28 eV are predominantly nonbonding, i.e. lone-pair like, as should be. The states above the Fermi level are clearly antibonding for all interactions around Sn3 (Fig. 4b–d) while for the Sn2–Sn2 interactions they remain nonbonding. The lowest-lying antibonding states 91 ˚ for are for the longest bond in the structure, 3.108(1) A Sn3–Sn3 (Fig. 4d). 4. Conclusions A new ternary Zintl phase, Ba 3 Li 4 Sn 8 , has been synthesized and structurally characterized. Its structure consists of chains made of edge-sharing cyclodecane-like units of tin in their ‘all-chair’ conformations. The Li 1 and Ba 21 cations screen the chains from each other and provide the extra electrons needed for chemical bonding and the compound is electronically balanced. However, the compound shows temperature-independent paramagnetism, Fig. 4. COOP curves for the four different Sn–Sn bonds in Ba 3 Li 4 Sn 8 : (a) Sn2–Sn2; (b) Sn1–Sn3; (c) Sn2–Sn3; (d) Sn3–Sn3. 92 S. Bobev, S.C. Sevov / Journal of Alloys and Compounds 338 (2002) 87 – 92 which is most likely due to either van Vleck paramagnetism due to a very small band gap of 0.3 eV, or because of actual overlap of the conduction and valence bands. [4] [5] [6] [7] [8] [9] Acknowledgements We thank the Petroleum Research Fund, administered by the ACS, for the financial support of this research. References ´ [1] V. Queneau, S.C. Sevov, Angew. Chem. Int. Ed. Engl. 36 (1997) 1754. ´ [2] V. Queneau, E. Todorov, S.C. Sevov, J. Am. Chem. Soc. 120 (1998) 3263. ´ [3] V. Queneau, S.C. Sevov, Inorg. Chem. 37 (1998) 1358. [10] [11] [12] [13] [14] [15] [16] [17] [18] [19] E. Todorov, S.C. Sevov, Inorg. Chem. 37 (1998) 3889. J.D. Corbett, Chem. Rev. 85 (1985) 383. J.D. Corbett, Angew. Chem. Int. Ed. 39 (2000) 670. S. Bobev, S.C. Sevov, Angew. Chem. Int. Ed. 39 (2000) 4108. S. Bobev, S.C. 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